An experiment was carried out to investigate the effect of concentration on the reaction: BrO₂ (aq) + 5 Br (aq) + 6 H* (aq) 3 Br₂ (1) + 3 H₂O (1) The following data was obtained: Initial [BrO3] Initial [Br] Initial [H*] Initial Rate Trial (mol/L) (mol/L) (mol/L) (mol/L's) 1 0.10 0.10 0.10 8.0 x 10-4 2 0.20 0.10 0.10 1.6 x 10-3 3 0.20 0.20 0.10 3.2 x 10-3 4 0.10 0.10 0.20 3.2 x 10-3 a) Deduce and state the rate law equation for this reaction. Show your process/reasoning. b) Calculate the value of k, the rate constant with correct units.

An experiment was carried out to investigate the effect of concentration on the reaction: BrO₂ (aq) + 5 Br (aq) + 6 H* (aq) 3 Br₂ (1) + 3 H₂O (1) The following data was obtained: Initial [BrO3] Initial [Br] Initial [H*] Initial Rate Trial (mol/L) (mol/L) (mol/L) (mol/L's) 1 0.10 0.10 0.10 8.0 x 10-4 2 0.20 0.10 0.10 1.6 x 10-3 3 0.20 0.20 0.10 3.2 x 10-3 4 0.10 0.10 0.20 3.2 x 10-3 a) Deduce and state the rate law equation for this reaction. Show your process/reasoning. b) Calculate the value of k, the rate constant with correct units.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Activity: 1 Determining Reaction Orders from Rate Data PROBLEM: Many gaseous reactions occur in a car engine and exhaust system. One of these is NO (g) - CO(g) –- NO(g) + CO (g) rate = k(NOJ"(CO) Use the following data to determine the individual and overall reaction orders: Initial (NO] Initial [CO] (mol/L) Initial Rate Experiment (mol/L-s) (mol/L) 1 0.0050 0 10 0.10 0.080 0.40 0.10 0.0050 0. 10 0 20
For the reaction A2 (aq) + B2 (aq) - 2 AB (ag) The initial rate of appearance of AB was 3.0 M/s. What is the general rate of reaction in M/s? Your Answer: Answer
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arrow_forward Step 3: solution b #(b): The overall chemical equation can be obtained by adding the three elementary step reactions and canceling the common species like "Pt(s)", "Cl(g)" and "ClCO(g)" (i): Cl2(g) + Pt(s) 2Cl(g) + Pt(s) (ii): Cl(g) + CO(g) + Pt(s) ClCO(g) + Pt(s) (iii): Cl(g) + ClCO(g) Cl2CO(g) ---------------------------------------------------------------- Adding the above 3 equations and canceling the common species like "Pt(s)", "Cl(g)" and "ClCO(g)" gives: Overall chemical equation, Cl2(g) + CO(g) Cl2CO(g) (Answer) arrow_forward Step 4: Solution c and solution d #(c): Initial enthalpy, H(Initial) = 600 kJ The final enthalpy can be obtained by adding the enthalpies of all the 3 elementary reactions. Hence the final enthalpy, H(Final) = H(i) + H(ii) + H(iii) = - 950 kJ + 575 kJ - 825 kJ = -1200 kJ Overall change in enthalpy, H = H(Final) - H(Initial) = - 1200 kJ - 600 kJ = - 1800 kJ Overall change in enthalpy = - 1800 kJ (Answer) #(d):…
Be sure to answer all parts. The bromination of acetone is acid-catalyzed: H* CH,COCH, + Br; CH,COCH,Br +H + Br catalyst The rate of disappearance of bromine was measured for several different concentrations of acetone, bromine, and H ions at a certain temperature: Rate of ICH,COCH, Brz (M) Disappearance of Br (M/s) (M) (M) (1) 0.650 0.0650 0.0650 5.91 x 105 (2) 0.650 0.130 0.0650 5.91 x 10 5 (3) 0.650 0.0650 0.130 1.18 x 10 (4) 0.865 0.0650 0.260 3.14 x 10 (5) 0.865 0.0650 0.0650 7.86 x 105 (a) What is the rate law for the reaction? O rate-k[CH,COCH,(Br3l(H'] rate=k[CH,COCH,lIBr2|[H*) O rate=k[CH,COCH,J[BrH"] O rate-k{CH3COCH,J[Br2|[H? rate=k(CH,COCH,l[Br,l[H
Question 1 of 6 Submit Which of the following represents the rate at which clo,-(aq) is appearing in the reaction below? 2 Clo,(aq) + 2 OH-(aq) → ClO,-(aq) + CIO, (aq) + H20(1) A) +1/2Δ[CIOJ/Δt B) -A[H,O]/At C) +A[0H¯]/At D) +1/2A[OH-]/At E) +A[CIO;-]/At
5. [30 pts] Two short questions on previous topics: A. The following two-step mechanism has been proposed for a certain aqueous reaction Step 1: ClO + ClO → ClO2+ Cl Step 2: ClO2 + CIO→ ClO3 + Cl¯ i. Write down the balanced equation for the overall (net) reaction. ii. Laboratory experiments give the following rate law for the reaction above: Rate = k[CIO¯]² If the two-step mechanism above is correct, which is the slow step? Explain your answer based on the laboratory result. B. Draw Lewis structures for the molecules below, and show the hydrogen-bonding interaction between the two molecules using a (...) symbol. ii. iii. i. CH2=O and H₂O CH3OH and CH3OH HF and HCN Hint: the atoms of HCN are connected in the order written.
5. Chlorine dioxide reacts in alkaline solution according to the equation 2CIO2 (aq) + 2OH- (aq) CIO3 (aq) + CIO2 (aq) + H20 (1) The experimental data of the reaction are given in the table below: [CIO2] (mol dm3) 0.07 [OH] (mol dm³) 0.184 Initial rate (mol dm-3 s-1) Experiment 1 0.016 0.14 0.184 0.064 0.28 0.368 0.512 a) Determine the rate law equation for the above reaction. b) Calculate the rate constant, k and state its unit. c) Calculate the rate of reaction when the concentrations of CIO2 and OH are 0.23 mol dm3 and 0.37 mol dm3, respectively.
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Consider this initial rate data at a certain temperature in the table for the reaction OH (aq) OCI (aq) + I (aq) OI (aq) + Cl(aq) Determine the rate law. rate k [OC] (1) Answer Bank (1-1² [OH Trial 1 2 3 4 [I Jo [OCI ]o (M) [OH lo (M) (M) 0.00171 0.00171 0.510 0.00171 0.00299 0.510 0.00279 0.00171 0.643 0.00171 0.00299 0.826 [OCI"] [OH-] Initial rates (M/s) 0.000359 0.000629 0.000465 0.000388
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